#2N_2H_4(l) + N_2O_4(l) -> 3N_2(g) + 4H_2O(l)#. If 10.81 g of #N_2H_4# is used, what mass of nitrogen is produced?

Your response is 14.188 grams of nitrogen gas.

To find the mass of nitrogen produced, we need to use stoichiometry based on the balanced chemical equation provided.

First, we need to determine the molar mass of N₂, which is 28.02 g/mol.

Then, we calculate the moles of N₂H₄ used:

moles of N₂H₄ = mass of N₂H₄ / molar mass of N₂H₄ moles of N₂H₄ = 10.81 g / 32.05 g/mol moles of N₂H₄ ≈ 0.337 mol

According to the balanced equation, 2 moles of N₂H₄ produce 3 moles of N₂. So, we can find the moles of N₂ produced:

moles of N₂ = (moles of N₂H₄ × 3) / 2 moles of N₂ = (0.337 mol × 3) / 2 moles of N₂ ≈ 0.506 mol

Finally, we calculate the mass of nitrogen produced:

mass of N₂ = moles of N₂ × molar mass of N₂ mass of N₂ = 0.506 mol × 28.02 g/mol mass of N₂ ≈ 14.18 g

Therefore, approximately 14.18 grams of nitrogen is produced when 10.81 grams of N₂H₄ is used.